Energy Changes

Cards (44)

  • Energy profile diagram for an exothermic reaction
    • Label the axis: energy
    • Label the reactants and products
    • Label the activation energy
    • Label the energy change
  • Bonds
    • Contain two chemical symbols separated by either a single, double or triple line
    • The chemical symbols can be the same or they could be different
  • Identifying bonds
    Count the number of each band you can repeatedly see
  • The number at the front of a molecule tells you there are 'X' number of the molecules present in the reaction (X is any number)
  • Bond Energy Calculations
    • Can be used to explain why energy changes take place
    • Old bonds are broken in reactants
    • New bonds are formed in products
  • Breaking chemical bonds

    Energy is supplied (taken in), therefore this is an endothermic process
  • Forming new bonds
    Energy is released, therefore this is an exothermic process
  • Bond energies are always positive
  • Bond energies are measured in kJ/mol
  • Calculating overall energy change
    Difference between the sum of the energy needed to break bonds in the reactants and the sum of the energy released when bonds in the products are formed
  • What happens to energy during chemical reactions?
    Energy is transferred to or from surroundings
  • What is an exothermic reaction?
    It is accompanied by a temperature rise
  • Give an example of an exothermic reaction.
    Combustion
  • How are exothermic reactions used in products?
    They are used in self-heating cans and hand warmers
  • What characterizes an endothermic reaction?
    It is accompanied by a fall in temperature
  • Provide an example of an endothermic reaction.
    Thermal decomposition
  • What happens in a reversible reaction that is exothermic in one direction?
    It is endothermic in the opposite direction
  • What is the independent variable in the required practical?
    The metal used
  • What is the dependent variable in the required practical?
    The temperature change
  • What are control variables in the experiment?
    Type, concentration, and volume of acid
  • What does measurement uncertainty imply?
    There is variability in the results obtained
  • What correlation should be observed in the experiment?
    The more reactive the metal, the greater the temperature change
  • How is the mean temperature change calculated?
    By averaging the recorded temperature changes
  • What is a key safety consideration in the experiment?
    Use eye protection due to corrosive acid
  • What is an accurate measurement?
    Close to the true value
  • What does it mean for results to be precise?
    Results are all close together
  • What does repeatability of results indicate?
    Similar results from the same experimenter
  • What does reproducibility of results indicate?
    Similar results from different experimenters
  • What is activation energy?
    The minimum energy needed for a reaction
  • How do energy level diagrams represent exothermic reactions?
    Products have less energy than reactants
  • How do energy level diagrams represent endothermic reactions?
    Products have more energy than reactants
  • What effect do catalysts have on activation energy?
    Catalysts reduce the activation energy needed
  • What happens to heat energy in exothermic reactions?
    It is transferred to the surroundings
  • What happens to heat energy in endothermic reactions?
    It is taken in from the surroundings
  • How can energy changes in reactions be measured?
    By mixing reactants in an insulated container
  • What is required to break a chemical bond?
    Energy is required to break a bond
  • What happens when a new chemical bond is formed?
    Energy is given out
  • What determines if a reaction is endothermic or exothermic?
    Comparison of energy required and released
  • What are the characteristics of endothermic and exothermic reactions?
    • Exothermic:
    • Temperature rises
    • Heat energy is released
    • Examples: combustion, rusting, neutralisation
    • Endothermic:
    • Temperature falls
    • Heat energy is absorbed
    • Examples: thermal decomposition, citric acid and sodium hydrogen carbonate
  • What are the steps involved in measuring energy changes in a chemical reaction?
    1. Set up equipment
    2. Measure initial temperature
    3. Add reactants and stir
    4. Record highest temperature reached
    5. Calculate temperature change
    6. Repeat with different reactants